Question

How much energy is required to melt these quantities of ice?
a. 56 g
b. 56 mol

Answer 1

The enthalpy is the amount of energy required to change from solid to liquid.

The molar enthalpy of fusion (kJ/mol) is 6.01 kJ/mol.

We can answer B first, since solving for A would require us to find moles, which takes more time.

q = H*n
q = 6.01*56
q = 336.56 kJ

On to a.

Since we know the molar enthalpy of fusion, we need to solve for the number of moles in 56 grams of ice.

n = 56/(16.00 + 2(1.008))
n = 3.108 mol

Now we can solve.

q = H * n
q = 6.01 * 3.108
q = 18.7 kJ


Answers:
a. 18.7 kJ
b. 336.56 kJ

Let me know if you'd like me to explain anything I did here.

-T.B.

Answer 2

The heat of fusion of ice is about 1807 J or 337 kJ

What is melting?

Melting is also called fusion. It is the process by which solid is changed into liquid. Ice can be changed from solid to liquid.

For the fusion of 56 g of ice;

H= mL

H= 56 g * 334 J/g = 18704 J

For the fusion of 56 mol;

H= 56 * 6.01 Kj/mol = 337 KJ

Learn more about heat of fusion: https://brainly.com/question/19579959

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